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What is the ideal acid test ratio?
some where between 1 to 1.5
What is the main reason between current ratio and acid test ratio?
The main difference between the current ratio and the acid-test ratio lies in the assets they consider. The current ratio includes all current assets, such as inventory, while the acid-test ratio excludes inventory and focuses only on the most liquid assets (cash, marketable securities, and receivables). This makes the acid-test ratio a more stringent measure of a company's short-term liquidity, as it assesses the ability to meet current liabilities without relying on inventory sales. Thus, the acid-test ratio provides a clearer picture of immediate financial health.
The acid test ratio does not include?
acid test / quick ration = quick assets / quick liablities quick assets = current assets - stock- prepaid expenses quick liablities = current liablities - bank overdraft
What does the acid test ratio not include cash or accounts receivable or supplies or inventory?
inventory
What are some types of liquidity ratios?
current and quick ratios. The quick (acid test) ratio is a more accurate measure of liquidity because it excludes inventories.
What is the pH of a .12 M solution of monochloroacetic acid?
The pH of a .12 M solution of monochloroacetic acid can be calculated using the equation pH = pKa + log([A-]/[HA]), where pKa for monochloroacetic acid is about 2.83. The concentration of A- (chloroacetate ion) can be found by multiplying the initial molarity by the degree of dissociation. Once these values are plugged into the equation, the pH can be determined to be around 2.78.
Why acetic acid is weaker than monochloro acid?
Acetic acid (CH3COOH) is weaker than monochloroacetic acid (ClCH2COOH) because the presence of a chlorine atom in monochloroacetic acid increases the electron-withdrawing effect, making the carboxylic acid group more acidic by stabilizing the negative charge on the conjugate base. This stabilization leads to easier dissociation of the proton, resulting in stronger acidity.
What is the clasification of monochoroacetic acid?
Chloroacetic acid, industrially known as monochloroacetic acid (MCA) is the organochlorine compound with the formula ClCH2CO2H. This carboxylic acid is a useful building-block in organic synthesis.
How do you prepare fatty acid from tartaric acid?
reduction
Why trichloroacitic acid is stronger than dichloro and monochloro acitic acid?
Trichloroacetic acid is stronger than dichloroacetic and monochloroacetic acids because it has more chlorine atoms attached to the central carbon, making it more electron-withdrawing and acidic. This extra electron withdrawal stabilizes the conjugate base formed after donating a proton, leading to stronger acidity.
How do you prepare buffer solution?
To prepare a buffer solution which may be acidic. Titrate ethanoic acid (weak acid) with sodium ethanoate(salt).
How do you prepare oxalic acid?
how do prepare 0.1 N Oxalic acid
What acid is used to prepare potassium chloride?
2K + 2HCl -> 2KCl + H2 hydrochloric acid would do here.
How do you prepare .1N phosphoric acid?
To prepare 0.1N phosphoric acid, you can dilute a more concentrated phosphoric acid solution, such as 85% phosphoric acid, to achieve the desired concentration. Measure the volume of the concentrated acid needed based on the final volume you want to prepare, then dilute it with distilled water accordingly. Ensure to use appropriate safety precautions and equipment when working with acids.
How do you prepare 0.1 phosphoric acid?
To prepare 0.1 phosphoric acid solution (w/v), dissolve 0.1 g of phosphoric acid in 100 mL of water. Stir the solution until the acid is completely dissolved. Remember to handle phosphoric acid with caution as it is a corrosive substance.
What is the proper way to prepare an acid solution?
Add the acid to the water, not the other way around.
How do you prepare 50 mM Sulphuric acid solution?
To prepare a 50 mM Sulphuric acid solution, you would need to calculate the required volume of concentrated Sulphuric acid (typically 96-98%) needed to dilute in water to achieve the desired concentration. You can use the formula: C1V1 = C2V2, where C1 is the concentration of the concentrated acid, V1 is the volume of concentrated acid needed, C2 is the desired concentration (50 mM), and V2 is the final volume of the solution you want to prepare.
